Can a zinc spoon be used to stir a solution of copper sulphate? Support your answer with reason
`E_(Zn^(2+)|Zn)^@=-0.76V`, `E_(Cu^(2+)|Cu)^@=+0.34V`

Can a nickel spoon be used to stir a solution of copper sulphate ? Support your answer with reason. [E^(@)(Ni^(2+)//Ni)= -0.25V,E^(@)(Cu^(2+)//Cu)=+0.34V]

Write the Nernst equation for the above cell, if E^@(Zn^(2+)|Zn)=-0.76V, E^@(Cu^(@+)|Cu)=+0.34V

A Galvanic cell consits of three compartment as shown in figure. The first compartment contain ZnSO_4 (1M) and III compartment contain CuSO_4 (1M). The mid compartment contain NaNO_3 (1M). Each compartment contain 1L solution: E_(Zn^(2+)//Zn)^(@)=-0.76 , E_(Cu^(2+)//Cu)^(@)=+0.34 , The concertation of Zn^(2+) in first compartment after passage of 0.1 F charge will be:

Can we store copper sulphate solution in iron vessel? Give suitable explanation in support of your answer [E°(Cu^(2+)//Cu)=+0.34V,E°(Fe^(2+)//Fe)=-0.44V]

Calculate the EMF of the cell, containing nickel and copper electrodes. Given E^@(NI^(2+)|NI)=-0.25V and E^@(Cu^(2+)|Cu)=+0.34V .

Can Chlorine gas be stored in Copper Cylinder ? Given E_(Cu^(+)//Cu)^(@)= 0.34V and E_(Cl_(2)//Cl)^(@)= 1.36V

A copper silver cell is set up. The copper ion concentration is 0.10 M. the concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. Given: E_(Ag^+|Ag)=+0.80V , E_(Cu^(2+)|Cu)=+0.34V

Calculate the standard Gibbs energy for the cell : Zn(s)+Zn^(2+)(aq)||Cu^(2+)(aq)|Cu(s) E_((Zn^(2+)//Zn)^(@))=-0.76V,E_((Cu^(2+)//Cu))^(@)=0.34V , F=96500 C .